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The recommended daily dose of calcium is 1200 mg. Calcium supplements often use calcium carbonate, $CaCO_3$, as the source of calcium. What mass of $CaCO_3$ should be used in a tablet so that one tablet provides the recommended daily dose of calcium?
$"Moles of calcium"$ $=$ $(1200xx10^-3*g)/(40.08*g*mol^-1)$ $=$ $0.04008*mol$. And thus we need $0.04008*mol$ $"calcium carbonate"$, i.e. a mass of $0.04008*molxx100.09*g*mol^-1$ $=$ $??g$.
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Sodium chloride is $NaCl$, and sodium sulfide is $Na_2S$. Why are there more sodium ions in the sulfide compound?
Sodium chloride is composed of $Na^+$ ions and $Cl^-$ ions. Now of course salt is neutral; and to ensure this sodium ion and chloride ions combine 1:1. On the other...
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Decomposing calcium carbonate yields calcium oxide and dioxide. What information is needed to calculate the mass of calcium oxide that can produced from 4.7 kg of calcium carbonate?
The balanced chemical equation The molar mass of $"CaCO"_3$ The molar ratio of $"CaO"$ to $"CaCO"_3$ The molar mass of $"CaO"$ Your strategy has four steps:...
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Calcium carbonate decomposes to form calcium oxide and carbon dioxide gas. If 44.5 grams of calcium oxide is produced, how many grams of calcium carbonate had to decomposez?
We need a stoichiometric reaction that represents the decomposition of calcium carbonate: $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g)uarr$ And thus calcium oxide and calcium carbonate are present in equimolar...
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The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produces 34.5 g of sodium upon decomposition. How much fluorine (in grams) forms?
The idea here is that you need to use the given mass ratio to determine how much fluorine will be produced if the also produces $"34.5 g"$ of sodium....
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A mixture of magnesium carbonate and magnesium oxide of mass $12.46*g$ underwent fierce heating. After heating, there were $8.43*g$ of salt remaining. What were the masses of magnesium carbonate, and magnesium oxide in the original sample?
$MgCO_3(s)+DeltararrMgO(s) + CO_2(g)$ And we would have to heat the magnesium salt VERY fiercely to get complete decarboxylation. $"Moles of carbon dioxide LOST"$ $=$ $(4.40*g)/(44.01*g*mol^-1)$ $=0.010*mol$ And therefore in...
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Calcium oxide and carbon dioxide are produced from the decomposition of calcium carbonate. How many moles of calcium carbonate are needed to produce 15.0 grams of the calcium oxide?
We interrogate the stoichiometric equation...... $CaCO_3(s) + Delta rarr CaO(s) + CO_2(g) uarr$ We require a molar quantity of $(15.0*g)/(56.08*g*mol^-1)=0.268*mol,$ with respect to $"calcium oxide"$. And clearly, we need a...
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Hydrochloric acid (HC) and sodium fluoride (NaF) react to produce hydrogen fluoride (HF) and sodium chloride (NaCl). How many moles of HF are produced per mole of HCl used?
The balanced equation for this reaction: $HCl (aq) + NaF (aq) rarr HF (aq) + NaCl (aq)$ We can see that the number of moles of $HCl$ is equal to...
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How many grams of sodium sulfide are formed if 1.50 g of hydrogen sulfide is bubbled into a solution containing 2.00 g of sodium hydroxide, assuming that the sodium sulfide is made in 94.0 % yield?
The first step for any chemical reaction is to write out the chemical equation to determine the molar ratios of the reactants and products. Then we will use the molecular...
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Calcium chloride dissolves in water to form calcium and chloride ions, producing 83kJ of heat per mole. Calculate final temp. when 0.02 moles of calcium chloride is dissolved into 150ml of water at a temperature initially of 19 degrees?
Given: The process of dissolving $CaCl_2$ in releases $(8.3xx10^4"J")/("mole of "CaCl_2)$ Compute the heat energy released for $0.02"mole of "CaCl_2$: $(8.3xx10^4"J")/(cancel("mole of "CaCl_2))(0.02cancel("mole of "CaCl_2))/1 = 1660"J"$ This heat energy...
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